Chapter 14, Problem 14.79QP

(1)

Interpretation Introduction

Interpretation:

The reaction which has greater activation energy has to be identified from the given diagram.

Concept introduction:

Arrhenius equation:

Arrhenius equation is a formula that represents the temperature dependence of reaction rates

The Arrhenius equation can be represented as follows

$k=A{e}^{-E_a/RT}$

$E_a$ is the activation energy ( it is the amount of energy needed to start reaction) and it’s unit is kJ/mol

R represents the universal gas constant and it has the value of 8.314 J/K.mol

T represents the absolute temperature

Slope in the graph of $\ln k$ (on Y-axis) with  $\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$T$}\right.$ (on X-axis) give activation energy of a reaction.

(2)

Interpretation Introduction

Interpretation:

The plot which corresponds to the higher temperature has to be identified.

Concept introduction:

Rate of the reaction is the change in the concentration of reactant or a product with time. It can be varied in accordance with temperature, pressure, concentration, presence of catalyst, surface area…

Generally rate of the reaction increases with increasing temperature.

Order of a reaction:  The sum of exponents of the concentrations in the rate law for the reaction is said to be order of a reaction.

Half-life is the time required for one half of a reactant to react.

For first order reaction $-kt=\ln \left(\frac{\left[A\right]}{\left[A_0\right]}\right)$

$\left[A\right]$ is the concentration of reactant A at time t ${\left[A\right]}_0$ is the  initial concentration of reactant, k is the rate constant.

The slope of a plot of $\ln \left[A\right]{}_t$ versus t equal to $-k$ .